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A galvanic cell with
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Chemistry
- The cell potential for the cell with the reaction Zn(s) + 2H+ (X M)→ Zn²+(2.5M) + H₂(4.5 M) is observed to be 0.445V. What is the pH in the H+ /H₂ half-cell? (& cell = 0.76V) 7.00 4.80 (Correct answer) 1.43 9.69 19.4arrow_forwardhello i need help with part a and b 1a) The standard reduction potential for the half-reaction Sn4+ + 2e- --> Sn2+ is +0.15 V.Consider data from the table of standard reduction potentials for common half-reactions in the table attached below.For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. write yes or no beside each one. Pb2+ + 2e- --> Pb Sn2+ + 2e- -->Sn 2H2O + 2e- --> H2 + 2OH- 2H+ + 2e- --> H2 Fe3+ + 3e- --> Fe PbSO4 + 2e- --> Pb + SO42- 1b) The standard reduction potential for the half-reaction: Sn4+ + 2e- --> Sn2+ is +0.15 V.Consider data from the table of standard reduction potentials for common half-reactions, in the table attached below. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of…arrow_forwardThe standard reduction potential voltage is associated with a reduction reaction at an electrode when all solutes are 0.10 M and all gases are at 0.1 atm. Group of answer choices True Falsearrow_forward
- Multi-Concept Problem 19.117 At 25 °C, a galvanic cell was set up having the following half-reactions. Fe2+(aq) + 2eS Fe(s), E°Fe2+ Cu2+(aq) + 2e S Cu(s), E°cu2+ = -0.447 V = +0.3419 V The copper half-cell contained 100 mL of 3.85 M CuSO4. The iron half-cell contained 31.6 mL of 0.312 M FeSO4. To the iron half-cell was added 43.5 mL of 0.662 M NaOH solution. The mixtu was stirred and the cell potential was measured to be 1.175 V. Calculate the value of Ksp for Fe(OH),. Ksp the tolerance is +/-2% Click if you would like to Show Work for this question: Open Show Workarrow_forwardStudent A prepared a concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]2- as the source of bromide ions. On the other hand, Student B prepared a galvanic cell (H), where the bromide ion concentration in the anode is equal to that in the cathode of cell L. Cell L Pt | Br2 | Br- (1.0 M) || Br- (x M) from [PbBr4]2- | Br2 | Pt Cell H Pt | Br2 | Br- (x M) || BrO3- (0.43 M), H+ (1.00 M) | Br2 | Pt Given: E° for the reduction of Br2 to Br- = +1.07 V > Given that the electrochemical cell L gives a potential of 0.0570 V, determine the concentration of bromide ions present in its cathode half-cell.> Given: Equilibrium concentration of Pb2+ in the cathode of L = 0.15 M and Equilibrium concentration of [PbBr4]2- in the cathode of L = 0.32 M. Determine the equilibrium constant for the formation of [PbBr4]2-.> Given that the electrochemical cell H gives a potential of 0.350 V, determine the standard potential for the reduction of BrO3- to…arrow_forwardThe free energy change for the following reaction at 25 °C, when [Ni=1.14 M and [Cd2+]=5.77x10 M, is -42.6 kJ: %3D Ni*(1.14 M) + Cd(s) Ni(s) + Cd2+ (5.77x10 M) AG=-42.6 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?arrow_forward
- Nernst Equation A concentration cell is constructed of two hydrogen electrodes one immersed in a solution with H^+= 1.0 M and the other in 0.65 M KOH. c) Determine Ecell for the reaction that occurs. d) Compare this value of Ecell with E° for the reduction of H20 to H2(g) in basic solution, and explain the relationship between them.arrow_forwardissue 17Suppose you want to build a galvanic cell where the half-reaction at the cathode is: Fe3+(aq) + e- → Fe2+(aq) Choose a half-reaction that would take place at the anode. The choice is yours. Suggest substances that would form the electrodes of this cell.arrow_forwardQuestion: Calculate the (a) electrical energy, (b) G and (c) K of the two galvanic cells in the following information below at standard-state condition Analyze and answer the following. 1. A galvanic cell consists of Mg anode in a 1.0 M Mg(NO3)2 and Al cathode in a 1.OM Al(NO3)3 solution with NaCl as the electrolyte in the salt bridge. 2. A galvanic cell is made of Tin anode in 1.0 M SnCl2 and iron cathode in a 1.0 M FeC12 solution with NANO3 as the electrolyte in the salt bridge.arrow_forward
- When the Cu²+ concentration is 6.78x104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 1.006V. What is the Zn2+ concentration? Cu²+ (aq) + Zn(s) Cu(s) + Zn²+ (aq) Answer: Submit Answer Retry Entire Group 6 more group attempts remainingarrow_forwardCHEMWORK Choose the statements that are correct. (Select all that apply.) O In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. Copper metal can be oxidized by Ag*. O Gold is a more active metal (better reducing agent) than silver. In a cell employing the half reactions Al3+ + 3e → Al and Mg2+ + 2e → Mg, aluminum functions as the anode. In a concentration cell electrons always flow from the compartment with the lower concentration to the compartment with the higher concentration.arrow_forwardPlz give answer asap Be sure to answer all parts. A galvanic cell is constructed as follows. One half-cell consists of a platinum wire immersed in a solution containing 1.00 M Sn2+ and 1.00 M Sn4+. The other half-cell has a thallium rod immersed in a solution of 1.00 M Tl+. (a) Write the half-cell reactions and the overall reaction. (Include states of matter. Enter the number of electrons in the following format #e−; e.g., 2e−, 4e−, etc.) Sn4+(aq) + → Tl(s) → → ( b)What is the equilibrium constant at 25°C?(E o Tl+ / Tl = −0.34 V.) × 10 Enter your answer in scientific notation. (c) What is the cell voltage if the Tl+ concentration is increased 13−fold? Varrow_forward
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